Answer:
% (COOK)2H2O = 37.826 %
Explanation:
mix: (COOK)2H2O + Ca(OH)2 → CaC2O4 + H2O
∴ mass mix = 4.00 g
∴ mass (CaC2O4)H2O = 1.20 g
∴ Mw (COOK)2H2O = 184.24 g/mol
∴ Mw (CaC2O4)H2O = 146.12 g/mol
∴ r = mol (COOK)2H2O / mol (CaC2O4)H2O = 1
- % (COOK)2H2O = (mass (COOK)2H2O / mass Mix) × 100
⇒ mass (COOK)2H2O = (1.20 g (CaC2O4)H2O)×(mol (CaC2O4)H2O / 146.12 g (CaC2O4)H2O)×(mol (COOK)2H2O/mol (CaC2O4)H2O)×(184.24 g (COOK)2H2O/mol (COOK)2H2O)
⇒ mass (COOK)2H2O = 1.513 g
⇒ % (COOK)2H2O = ( 1.513 g / 4 g )×100
⇒ % (COOK)2H2O = 37.826 %
Answer:
0.0025 M/min
Explanation:
The rate of a reaction can be calculated for an element, based on its stoichiometric coefficient. For a reaction:
aA + bB = cC + dD , the rate will be
r = -(1/a)x(Δ[A]/Δt) = -(1/b)x(Δ[B]/Δt) = (1/c)x(Δ[C]/Δt) = (1/d)x(Δ[D]/Δt)
Where Δ[X] is the variation of the concentration of the X compound, Δt is the time variation, and the signal of minus in the reagents compounds is because they are disappearing, so Δ[X] will be negative, and r must be positive. So, for the reaction given:
r = -(1/2)x(Δ[NO]/Δt)
r = -(1/2)x( (0.025 - 0.1)/15)
r = 0.0025 M/min
Atomic number of F = 9
Electron configuration of F:-
⁹F = 1s² 2s² 2p⁵
Incase of F2: Total electrons: 9 + 9 = 18
For F2 the ground state electron configuration would be:
F2 = (1σ)²(1σ*)²(2σ)²(2σ*)²(2pσ)²(2pπ)⁴(2pπ*)⁴
Incase of F2+: There is loss of one electron from neutral F2. Total electrons: 18-1 = 17
For F2+ the ground state electron configuration would be:
F2 = (1σ)²(1σ*)²(2σ)²(2σ*)²(2pσ)²(2pπ)⁴(2pπ*)³
